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A bromate is a chemical compound that contains this ion. Examples of bromates include sodium bromate (NaBrO 3) and potassium bromate (KBrO 3). Bromates are formed many different ways in municipal drinking water. The most common is the reaction of ozone and bromide: Br − + O 3 → BrO − 3
Bromic acid, also known as hydrogen bromate, is an oxoacid with the molecular formula HBrO 3.It only exists in aqueous solution. [1] [2] It is a colorless solution that turns yellow at room temperature as it decomposes to bromine.
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [ 4 ] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
The Lewis acidity of all the gallium trihalides, GaBr 3 included, has been extensively studied thermodynamically, and the basicity of GaBr 3 has been established with a number of donors. [2] GaBr 3 is capable of accepting an additional Br − ion or unevenly splitting its dimer to form [GaBr 4] −, a tetrahedral ion of which crystalline salts ...
Potassium bromate is typically used in the United States as a flour improver (E number E924). It acts to strengthen the dough and to allow higher rising. It is an oxidizing agent, and under the right conditions, is reduced to bromide in the baking process.
FeBr 3 forms a polymeric structure featuring six-coordinate, octahedral Fe centers. [2] Although inexpensively available commercially, FeBr 3 can be prepared by treatment of iron metal with bromine: 2 Fe + 3 Br 2 → 2 FeBr 3. Above 200 °C, FeBr 3 decomposes to ferrous bromide: 2FeBr 3 → 2FeBr 2 + Br 2
Structure of N-bromosuccinimide, a common brominating reagent in organic chemistry. Like the other carbon–halogen bonds, the C–Br bond is a common functional group that forms part of core organic chemistry. Formally, compounds with this functional group may be considered organic derivatives of the bromide anion.
The most common Lewis bases are anions. The strength of Lewis basicity correlates with the pK a of the parent acid: acids with high pK a 's give good Lewis bases. As usual, a weaker acid has a stronger conjugate base. Examples of Lewis bases based on the general definition of electron pair donor include: simple anions, such as H − and F −